Question Paper

Topics: Chemical reaction, Rate equation, Mole Pages: 37 (6076 words) Published: July 1, 2013
CHEMISTRY (Theory)
Time allowed : 3 hours General Instructions: (i) All questions are compulsory. Maximum Marks : 70

(ii) Marks for each question are indicated against it. (iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark each. (iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks each. (v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks each. (vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each. (vii) Use Log Tables, if necessary, Use of calculators is not allowed.

QUESTION PAPER CODE 56/1/1 1. 2. 'Crystalline solids are anisotropic in nature.' What does this statement mean? Express the relation between conductivity and molar conductivity of a solution held in a cell. Define 'electrophoresis'. Draw the structure of XeF2 molecule. Write the IUPAC name of the following compound: (CH3)3 CCH2Br 6. 7. Draw the structure of 3-methylbutanal. Arrange the following compounds in an increasing order of their solubility in water: C6H5NH2, (C2H5)2NH, C2H5NH2 182

3. 4. 5.

8. 9.

What are biodegradable polymers? The chemistry of corrosion of iron is essentially an electrochemical phenomenon. Explain the reactions occurring during the corrosion of iron in the atmosphere. Determine the values of equilibrium constant (KC) and ∆G for the following reaction: o

10.

 Ni(s) + 2Ag+ (aq)  → Ni2+(aq) + 2Ag(s), E = 1.05 V o

(IF = 96500 C mol ) 11. 12. Distinguish between 'rate expression' and 'rate constant' of a reaction. State reasons for each of the following: (i) (ii) − The N – O bond in NO − is shorter than the N – O bond in NO 3 . 2

–1

SF6 is kinetically an inert substance. OR

State reasons for each of the following: (i) (ii) 13. All the P-Cl bonds in PCl5 molecule are not equivalent. Sulphur has greater tendency for catenation than oxygen.

Assign reasons for the following: (i) (ii) Copper (I) ion is not known in aqueous solution. Actinoids exhibit greater range of oxidation states than lanthanoids.

14.

Explain the following giving one example for each: (i) (ii) Reimer-Tiemann reaction. Friedel Craft's acetylation of anisole.

15.

How would you obtain (i) (ii) Picric acid (2, 4, 6-trinitrophenol) from phenol, 2-Methylpropene from 2-methylpropanol ?

183

16.

What is essentially the difference between α-form of glucose and β-form of glucose? Explain. Describe what you understand by primary structure and secondary structure of proteins. Mention two important uses of each of the following: (i) (ii) Bakelite Nylon 6

17.

18.

19.

Silver crystallizes in face-centered cubic unit cell. Each side of this unit cell has a length of 400 pm. Calculate the radius of the silver atom. (Assume the atoms just touch each other on the diagonal across the face of the unit cell. That is each face atom is touching the four comer atoms.) → Nitrogen pentoxide decomposes according to equation: 2N2O5(g)  4 NO2(g) + O2(g).

20.

This first order reaction was allowed to proceed at 40 °C and the data below were collected: [N2O5] (M) 0.400 0.289 0.209 0.151 0.109 (a) (b) (c) Time (min) 0.00 20.0 40.0 60.0 80.0

Calculate the rate constant. Include units with your answer. What will be the concentration of N2O5 after 100 minutes? Calculate the initial rate of reaction.

184

21.

Explain how the phenomenon of adsorption finds application in each of the following processes: (i) (ii) (iii) Production of vacuum Heterogeneous catalysis Froth Floatation process OR Define each of the following terms: (i) (ii) (iii) Micelles Peptization Desorption

22.

Describe the principle behind each of the following processes: (i) (ii) (iii) Vapour phase refining of a metal. Electrolytic refining of a metal. Recovery of silver after silver ore was leached with NaCN.

23.

Complete the following chemical equations: (i) (ii) (iii)
→ Mn O − + C2 O 2 − + H +  4 4

KMnO4 heated →  
 Cr2 O 2 −...
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